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Intro to Inorganic Chemical NomenclaturePart 1, Binary Compounds

This lesson was divided into two partsPart 1 Binary Compounds

• In this first video we are studying the nomenclature of Binary Compounds

• There is also a second video dealing with the nomenclature of Polyatomic Compounds.

• Youtube ‘Inorganic Chemical Nomenclature Part 2 Polyatomic Compounds’

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Intro to Inorganic Chemical NomenclaturePart 1 Binary CompoundsChemical Nomenclature = writing the formulas and names of chemicals.Using three systems of inorganic nomenclature …• the Stock system• the Prefix system• the Ous-Ic systemThis requires that you learn the names, formulas and oxidation numbers (Ox #’s) of a variety of monatomic elements and polyatomic ions needed for binary and polyatomic compounds.This lesson is designed for a 1st semester college chemistry student and assumes that the student already has a working knowledge of electron configuration, electronegativity, chemical bonding, and acid ionization.

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Intro to Inorganic Chemical NomenclatureChemical Formulas of Binary Compounds:

Binary compounds are made of two different kinds of atoms.

A chemical formula tells us which atoms and how many atoms of each kind are present in a chemical compound.

Look at the structure of a water molecule.

Each water molecule contains 2 hydrogen atoms and 1 oxygen atom.

A subscript of ‘1’ is never written in formulas.

Look at the formulas on the right and identify the error in each.

H 2Osym bol for hydrogen sym bol for oxygen

subscript indicates2 hydrogen atom s

im plied subscript of 1indicating 1 oxygen atom

H2O1

H2O(H)2OOH2

/

/ /

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1A               1H (2.1)

hydrogen

1-1 2A   3A 4A 5A 6A 7A

3Li (1.0)

lithium1---

4Be(1.5)beryllium

2---

 

5B (2.0)

boron3---

6C (2.5)

carbon2, 4-4

7N (3.0)

nitrogen

2,3,4,5-3

8O (3.5)

oxygen--- -2

9F (4.0)

fluorine----1

11Na (1.0)

sodium1---

12Mg (1.2)

magnesium

2---  

13Al

(1.5)aluminu

m

+3---

14Si

(1.8)silicon

4---

15P (2.1)phosphor

us

3, 4, 5-3

16S (2.5)

sulfur2, 4, 6

-2

17Cl

(3.0)chlorine1,3,5,7

-1

19K (0.9)potassium

1---

20Ca (1.0)

calcium2---

 

31Ga (1.7)

gallium3---

32Ge (1.9)

germanium

4---

33As

(2.1)arsenic

3, 5-3

34Se

(2.4)selenium

4, 6-2

35Br

(2.8)bromine

1, 5-1

37Rb (0.9)

rubidium1---

38Sr (1.0)strontium

2---

 

49In

(1.6)indium

1, 3---

50Sn

(1.8)tin2, 4---

51Sb (1.9)

antimony

3, 5-3

52Te

(2.1)tellurium

4, 6-2

53I (2.5)

iodine1, 5, 7

-1

55Cs (0.8)

cesium1---

56Ba (1.0)

barium2---

 

81Tl

(1.6)thallium

1, 3---

82Pb

(1.7)lead2, 4---

83Bi

(1.8)bismuth

3, 5---

84Po (1.9)

polonium

2, 4---

85At

(2.1)astatine

 

 

87Fr (0.8)francium

1---

88Ra (1.0)

radium2---

           

Electronegativity (EN) values of A-group Elements H2OEN: 2.1 (H) < 3.5 (O)

The less EN atom is listed first.

Practice:Write the formula of a compound made of …• one S & two Na atoms Na2S 1.0 (Na) < 2.5 (S)

• one P & three Br atoms PBr3 2.1 (P) < 2.8 (Br)

• two Cl’s & one Mg atom MgCl2 1.2 (Mg) < 3.0 (Cl)

In formulas of ionic compounds, symbols of metals precede nonmetals because all metals have lower EN values than any nonmetal.

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Chemical Formulas of Binary Compounds

Use the table of EN values to write the chemical formulas of the compounds shown below…

EN: Al (1.5) < O (3.5)

Al2O3

C (2.5) < O (3.5)

CO2

Ca (1.0) < F (4.0)

CaF2

Some Exceptions in Chemical Formulas of Binary CompoundsThe least Electronegative atom in binary compounds are usually listed first, but there are a few historical exceptions …• In the formulas of hydrocarbon compounds (abbreviated HC’s), which are

compounds containing only hydrogen and carbon, C (EN=2.5) is listed before H (EN=2.1), even though C has the higher EN value.

• Most formulas of binary compounds, in which H is listed first, are acids, such as hydrochloric acid, HCl and hydrofluoric acid, HF.

• HC’s are not acidic so their H’s are listed last.

CH4, methane, is the major component of natural gas.

C2H6, ethane is the 2nd largest component of natural gas

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More Exceptions in Chemical Formulas of Binary Compounds• In the formulas of binary compounds containing nitrogen, N is usually

listed first regardless of its EN value.

• Ammonia, NH3, is not acidic. It’s a moderately strong base.

• Listing H first would make ammonia look acidic … H3N

In ammonia, NH3, EN N (3.0) > H (2.1), but N is written first.

In N2O5, N (3.0) < O (3.5)N is less EN and written first.

/

/

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Naming Binary Compounds

There are three systems for naming binary compounds

1. The Stock System (the most comprehensive)e.g., sodium chloride

2. The Prefix System (for nonmetal compounds only)e.g., carbon monoxide, carbon dioxide

3. The ous-ic system (has limited use)e.g., ferrous oxide, ferric oxide

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The Stock System for Naming Binary CompoundsCaCl2 = calcium chloride Al2O3 = aluminum oxide

name of less EN atom first

name of more EN atom ends in ‘ide’

a space between

name of less EN atom first

name of more EN atom ends in ‘ide’

a space between

chlorine chloride oxygen oxide• In ionic compounds (made of metal cations, ⊕ and nonmetal anions, ⊖), the less

EN atom is a metal cation, and the more EN atom is a nonmetal anion.• The name of the metal cation is the same as the element’s name but the anion’s

name ends in ‘ide’.• Note that the Stock system name does not tell us the relative number of atoms in

the formula. This will be explained later.

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1A               8A 1H (2.1)

hydrogen

1-1 2A   3A 4A 5A 6A 7A

He

Helium

3Li (1.0)

lithium1---

4Be(1.5)beryllium

2---

 

5B (2.0)

boron3---

6C (2.5)

carbon2, 4-4

7N (3.0)

nitrogen

2,3,4,5-3

8O (3.5)

oxygen--- -2

9F (4.0)

fluorine----1

Ne

Neon

11Na (1.0)

sodium1---

12Mg (1.2)

magnesium

2---  

13Al

(1.5)aluminu

m

+3---

14Si

(1.8)silicon

4---

15P (2.1)phosphor

us

3, 4, 5-3

16S (2.5)

sulfur2, 4, 6

-2

17Cl

(3.0)chlorine1,3,5,7

-1

Ar

Argon

19K (0.9)potassium

1---

20Ca (1.0)

calcium2---

 

31Ga (1.7)

gallium3---

32Ge (1.9)

germanium

4---

33As (2.1)

arsenic3, 5-3

34Se

(2.4)selenium

4, 6-2

35Br

(2.8)bromine

1, 5-1

Kr

Krypton

37Rb (0.9)

rubidium1---

38Sr (1.0)strontium

2---

 

49In

(1.6)indium

1, 3---

50Sn

(1.8)tin2, 4---

51Sb (1.9)

antimony3, 5-3

52Te

(2.1)tellurium

4, 6-2

53I (2.5)

iodine1, 5, 7

-1

Xe

Xenon

Learn the anion names & charges.

hydride (-

1)

carbide

(-4)

nitride (-

3)

phosphide

(-3)

oxide (-2)

sulfide (-

2)

selenide

(-2)

fluoride (-

1)

chloride

(-1)

bromide

(-1)

iodide (-

1)

Nonmetal anions gain enough electrons to fill their valence shell to become isoelectronic with the nearest noble gas.

Anions typically have only 1 possible Ox #, which is easy to learn if you know their Group number on the PD table

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Practice naming these binary compounds using the Stock system:

K3P

MgO

Al2S3

Ca3N2

MgF2

LiI

Be2C

potassium phosphide

magnesium oxide

aluminum sulfide

calcium nitride

magnesium fluoride

lithium iodide

beryllium carbide

BaBr2

CaH2

Na2Se

SrCl2

B2O3

SiC

HF

barium bromide

calcium hydride

sodium selenide

strontium chloride

boron oxide

silicon carbide

hydrogen fluorideNote that the last three examples are not ionic compounds. They are composed of metalloids and/or nonmetals only, yet the Stock system names all compounds as if they were ionic. The less EN atom is first (using the atom’s name). The more EN atom is last (using the anion’s ‘ide’ name).

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Writing Chemical Formulas of Binary CompoundsIn order to write formulas and name compounds, you will need the ‘oxidation numbers’ (Ox #’s) of the atoms/ions in a compound.

Ox #’s are explained in detail in a video entitled ‘Oxidation Numbers’ and will only be discussed briefly in this lesson.

What is an oxidation number (Ox #)?Ox # is a charge assigned to an atom or ion in a compound.All pure elements have an Ox # = 0, e.g., Ox # Cu=0, H2=0, S8=0.About 20 elements have only one Ox # (fixed Ox #’s), other than 0, and they must be memorized, but it is easy to do so if you learn their position on the periodic table.The Ox #’s of other atoms/ions are calculated from the chemical formula.

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1H (2.1) hydrogen

1 -1 2A

Key

3A 4A 5A 6A 7A 3Li (1.0) lithium

1 ---

4Be(1.5) beryllium

2 ---

7N (3.0) nitrogen 2,3,4,5

-3

5B (2.0)

boron

3 ---

6C (2.5) carbon 2, 4 -4

7N (3.0) nitrogen 2,3,4,5

-3

8O (3.5) oxygen

--- -2

9F (4.0) fluorine

--- -1

11Na (1.0) sodium

1 ---

12Mg (1.2) magnesium

2 ---

3B

4B

5B

6B

7B

8B

8B

8B

1B

2B

13Al (1.5) aluminum

3 ---

14Si (1.8) silicon

4 ---

15P (2.1) phosphorus

3, 4, 5 -3

16S (2.5) sulfur 2, 4, 6

-2

17Cl (3.0) chlorine 1,3,5,7

-1

19K (0.9) potassium

1 ---

20Ca (1.0) calcium

2 ---

21Sc (1.3) scandium

3 ---

22Ti (1.4) titanium

3, 4 ---

23V (1.5)

vanadium

2,3,4,5

---

24Cr (1.6) chromium

2, 3, 6

---

25Mn (1.6) manganese

2,3,4,6,7

---

26Fe (1.7)

iron 2, 3 ---

27Co (1.7)

cobalt 2, 3 ---

28Ni (1.8)

nickel 2, 3 ---

29Cu (1.8)

copper 1, 2 ---

30Zn (1.6)

zinc 2 ---

31Ga (1.7) gallium

3 ---

32Ge (1.9) germanium

4 ---

33As (2.1)

arsenic 3, 5

-3

34Se (2.4) selenium

4, 6 -2

35Br (2.8) bromine

1, 5 -1

37Rb (0.9) rubidium

1 ---

38Sr (1.0) strontium

2 ---

39Y (1.2) yttrium

3 ---

40Zr (1.3) zirconium

4 ---

41Nb (1.5) niobium

3,5 ---

42Mo (1.6) molybdenum

2,3,4,5,6

---

43Tc (1.7) technetium

--- ---

44Ru (1.8) ruthenium

2,3,4 ---

45Rh (1.8) rhodium

2, 3, 4

---

46Pd (1.8) palladium

2, 4 ---

47Ag (1.9)

silver 1 ---

48Cd (1.6) cadmium

2 ---

49In (1.6) indium

1, 3 ---

50Sn (1.8)

tin 2, 4 ---

51Sb (1.9) antimony

3, 5

-3

52Te (2.1) tellurium

4, 6 -2

53I (2.5)

iodine 1, 5, 7

-1

55Cs (0.8)

cesium 1 ---

56Ba (1.0)

barium 2 ---

57La (1.1) lanthanum

3 ---

72Hf (1.3) halfnium

4 ---

73Ta (1.4) tantalum

5 ---

74W (1.5)

tungsten 2,3,4,5,6

---

75Re (1.7) rhenium 1,2,4,6,7

---

76Os (1.9) osmium 2,3,4,6,8

---

77Ir (1.9) iridium 2,3,4,6

---

78Pt (1.8) platinum

2, 4 ---

79Au(1.9)

gold 1, 3 ---

80Hg (1.7)

mercury

1, 2 ---

81Tl (1.6) thallium

1, 3 ---

82Pb (1.7)

lead 2, 4 ---

83Bi (1.8) bismuth

3, 5

---

84Po (1.9) polonium

2, 4 ---

85At (2.1) astatine

electronegativity (EN)

symbol & proton number

positive oxidation numbers

negative oxidation numbers

Fixed Ox #’s are highlighted (red and yellow). Metals cannot have Ox #’s (they never gain e’s).⊖Most nonmetals can have or Ox #’s, e.g., Cl in ICl (Cl = -1), Cl in ClF (Cl = +1), Cl in ClO⊖ ⊕ 2 (Cl = +4), Cl in ClF7 (Cl = +7).Note that the nonmetal with higher EN always gets a Ox #⊖ Fixed Ox #’s are easily memorized by knowing

their A-Group number on the PD table.Other Ox #’s can all be calculated.

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Writing the Formulas of Binary Compounds•Chemical formulas represent the smallest whole number ratio of atoms/ions in a compound.•The positive and negative charges (Ox #’s) must add up to zero; the charges balance.

Steps calcium chloride boron bromide hydrogen sulfide magnesium phosphide

4. Use subscripts to write the formulas BBr3 H2S Mg3P2

calcium: Ca+2

chloride: Cl-

1 Ca+2 ion for every 2 Cl- ions

CaCl2

Ca+2 = +2

Cl- -1 -1 = -2

1. Obtain ion symbols & Ox #’s (charges)

2. Find the total charge needed to balance + & - charges

3. Find the ratio of + and - ions

boron: B+3 (2.0EN)

bromide: Br - (2.8EN)

B+3

= +3

Br -

-1 -1 -1 = -3

1 B+3 ion for every 3 Br - ions

hydrogen: H+ (2.1EN)

sulfide: S-2 (2.5EN)

H+1 +1 +1 = +2

S-2 = -2

2 H+ ions for every 1 S-2 ion

magnesium: Mg+2

phosphide: P-3

Mg+2

+2 +2 +2 = +6

P-3

-3 -3 = -6

3 Mg+2 ions for every 2 P-3 ions

Nonmetals such as Cl, Br, H, S and P can have or Ox #’s. An atom is assigned a Ox # when it ⊕ ⊖ ⊕is the less EN atom in a compound and a Ox # when it is the more EN atom in a compound. ⊖

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Practice writing the chemical formulas of binary compounds:name ions formula

magnesium oxidepotassium nitridebarium fluoridesilicon iodideberyllium carbidecalcium hydridelithium selenidesodium phosphidezinc phosphidealuminum sulfideboron oxide

Mg+2 O-2

K+ N-3

Ba+2 F-

Al+3 S-2

B+3 O-2

Si+4 I-

Be+2 C-4

Ca+2 H-

Li+ Se-2

Na+ P-3

Zn+2 P-3

MgO

K3N

BaF2

Al2S3

B2O3

SiI4

Be2C

CaH2

Li2Se

Na3P

Zn3P2

A chemical formula shows the lowest whole number ratio of ions such that the total positive and negative charges are equal.The ‘Inverse rule’ is an easy way to find this ratio.Consider zinc phosphide.

Zn+2 P-3 Zn3P2

The number of Zn cations (3) equals the charge of the anion (-3), and the number of P anions (2) equals the charge of the cation (+2).But remember to reduce this to the lowest whole number ratio.Consider beryllium carbide.

Be+2 C-4 Be4C2 Be2C

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Finding an Ox # in Compounds Containing a Multivalent Ion

water = H2O water ≠ HO2 or H3O or HO, etc.because the Ox # H = +1 and Ox # O = -2

In order to combine elements in a chemical formula in the correct ratio, you need to know the Ox #’s of each element. You will also need to know these Ox #’s for writing chemical names.However many elements are ‘multivalent’; they have more than one possible Ox #.Fortunately, it is always true that at least one of the elements in a binary compound will have an Ox # that is known for certain and so the other element’s Ox # can be calculated.Example 1: Manganese has 5 different Ox #’s in its compounds, i.e., +2, +3, +4, +6 and +7.Calculate the Ox # of Mn in MnCl2.

Answer: Mn = +2Here’s why: The Ox # of Cl is -1 because it is more EN than Mn. Chloride is always -1.The total negative charge in MnCl2 = (Cl-1 × 2) = -2.

So the total positive charge of Mn must be +2, and the Ox # of Mn must be +2.

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Example 2: Calculate the Ox # of Mn in Mn2O3

Answer: Mn = +3Here’s why: The Ox # of O is always -2.The total negative charge of three O’s = (-2 × 3) = -6The total positive charge of both Mn ions must be +6 (total = total ).⊕ ⊖So each Mn has a charge of (+6/2) = +3

or solve as a math equation:Let Ox # of Mn = xThe sum of all Ox #’s = 0Mn2O3 = 0(x)*2 + (-2)*3 = 02x – 6 = 0x = +6/2 = +3 Mn+3

or use the Inverse Rule:

Mn2O3

-2+3

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Practice: Calculate the Ox # of the underlined ion in each formula

Formula anion charge cation charge Formula anion charge cation charge

MnO2 Cu3P

MnO3 PbF4

Mn2O7 PCl5

V3N5 Mo2S5

Fe4C3 NiH3

-3-2-2-2-3-4

+4+6+7+5+3

-1-1-2-1 +3

+5+5+4+1

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Naming Binary Compounds Containing a Multivalent Ion:Iron (Fe), like manganese (Mn) can exhibit more than one Ox #. There are two kinds of iron chloride, FeCl2 and FeCl3. The name ‘iron chloride’ is thus ambiguous.

In binary compounds containing cations with more than one Ox #, the Ox # of the cation is written in Roman numerals (in parentheses) immediately after the cation. Thus FeCl2 is named iron(II) chloride and FeCl3 is named iron(III) chloride.

There are two different forms of iron chloride.Iron(II) chloride is green.Iron(III) chloride is yellow/rusty colored.Each different chemical compound must have its own, unique, unambiguous name.

Fe +2 C l-F eC l2 = = iron(II) chloride

Fe +3 C l-F eC l3 = = iron(III) chloride

n o sp a ce b e tw e e n th e ca tio n n a m e a n d its O x # b u t a lw a ys le a ve a sp a ce im m e d ia te ly b e fo re th e a n io n n a m e

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Look at the formulas and names of two kinds of iron oxide, FeO and Fe2O3.Please read carefully: The Ox # listed immediately after the cation indicates the charge on the cation, not necessarily the number of anions in the formula.

To name a compound, write the ion symbols and determine their Ox #’s from the combining ratio given in the formula. The anion usually has only one possible Ox #, so calculate the Ox # of the cation remembering that the total charge and charges in compounds are equal⊕ ⊖ .

F e +2 O -2F eO = = iron (II) oxide

F e +3 O -2F e 2O 3 = = iron (III) oxide

T he O x #, e .g., (II) or (III) ind icates the charge on the cation, not necessarily the num ber of an ions present.

FeO is black

Fe2O3 is rusty/red

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Naming Binary Compounds Containing a Multivalent Ion:

Steps Au3N Cl2O5

5. Write the name of the compound

1. Identify the Ox # that is known for certain (usually the anion’s).

2. If allowed, check the periodic table for the possible charges of the other ion.

3. Determine the ratio of ions in the formula

4. Find what charge must be on the multivalent ion to balance all charges

chlorine(V) oxide

nitride: N-3 (Group 5A)(N is more EN than Au, so it uses its negative Ox #)

Au+ or Au+3

Au3N means 3 gold ions for every 1 nitride ion.Au+ +1 +1 +1 = +3N-3 = -33 Au+ ions are needed for every 1 N-3 ion

gold(I) nitride

oxide: O-2 (Group 6A)O is more EN than Cl, O always has an Ox # of -2

Cl+, Cl+3, Cl+5 or Cl+7

Cl2O5 means 2 chlorines for every 5 oxide ions.Cl+5: +5 +5 = +10O 2-: -2 -2 -2 -2 -2 = -102 Cl+5 atoms are needed for every 5 O-2 ions.

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name formula ions name formula ions

FeO Fe2O3

CrO3 MnS2

NiF3 CoCl3

CuO CoO

Cu2O Sn3N4

AuBr3 Sn3N2

Fe+2 O-2

Cr+6 O-2

Ni+3 F-

Cu+2 O-2

Cu+ O-2

Au+3 Br-

Fe+3 O-2

Mn+4 S-2

Co+3 Cl-

Co+2 O-2

Sn+4 N-3

Sn+2 N-3

iron(II) oxide

chromium(VI) oxide

nickel(III) fluoride

copper(II) oxide

copper(I) oxide

gold(III) bromide

iron(III) oxide

manganese(IV) sulfide

cobalt(III) chloride

cobalt(II) oxide

tin(IV) nitride

Practice Naming Binary Compounds Containing a Multivalent Ion:Determine Ox #’s of the ions in the compounds below. Use these Ox #’s to write Stock system names of the compounds.

tin(II) nitride

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Practice Writing Formulas of Binary Compounds Containing Multivalent Ions:

name formula ions name formula ions

chromium(III) oxide cobalt(III) phosphide

nickel(II) fluoride vanadium(V) chloride

titanium(IV) oxide tungsten(IV) carbide

Cr+3 O-2

Ni+2 F-

Ti+4 O-2TiO2

NiF2

Cr2O3 CoP

VCl5

WC

Co+3 P-3

V+5 Cl-

W+4 C-4

Note: The formula of a binary compounds does not show the charge of the cation or the anion. Do not write any charges in binary compound formulas.For example, sodium chloride’s formula is NaCl, not Na+Cl-.

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Binary Acids:Binary acids contain hydrogen, H, that is covalently bonded to a non metal. Hydrogen chloride, HCl, is an example of a binary acid.When dissolved in water, hydrogen chloride is named hydrochloric acid because it releases an acidic H+ ion when it ionizes.Learn the names and formulas of the five common binary acids, listed below.

name (anhydrous) name (in water) formula reaction in water

HF

HCl

HBr

HI

H2S

hydrogen fluoride

hydrogen chloride

hydrogen bromide

hydrogen iodide

hydrogen sulfide

hydrofluoric acid

hydrochloric acid

hydrobromic acid

hydroiodic acid

hydrosulfuric acid

HF H+ + F-

HCl H+ + Cl-

HBr H+ + Br-

HI H+ + I-

H2S 2H+ + S-2

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Summary of Stock System Nomenclature for Binary Compounds

SnO tin(II) oxide NaCl sodium chloride

SnO2 tin(IV) oxide CaCl2 calcium chloride

Cr2O3 chromium(III) oxide Al2O3 aluminum oxide

CrO3 chromium(VI) oxide ZnS zinc sulfide

CuBr copper(I) bromide Ag3P silver phosphide

CuBr2 copper(II) bromide

There is > 1 tin oxide, chromium oxide, copper bromide. Sn, Cr, Cu have > 1 Ox # Sn (+2, +4), Cr (+2, +3, +6), Cu (+1, +2) Ox #’s must be included in the name (written in Roman numerals).

There is only one sodium chloride, calcium chloride, aluminum oxide, zinc sulfide, and silver phosphide. Na, Ca, Al, Zn, Ag have only 1 Ox # each.Na & Ag (+1), Ca & Zn (+2), Al (+3) The Ox # is not stated in the name.

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The Prefix System for Binary CompoundsFor binary compounds containing two non-metals, a Greek or Latin prefix is attached to the name of an element to indicate the number of atoms of that element in the compound.

Number123456

FormulaCOCO2

SO3

CCl4

PCl5

SF6

Prefix System Namecarbon monoxidecarbon dioxidesulfur trixodecarbon tetrachloridephosphorus pentachloridesulfur hexafluoride

Prefixmonoditritetrapentahexa

7 = hepta, 8 = octa, 9 = ennea, 10 = decaAlthough this system is used almost exclusively for non-metal/non-metal compounds, occasionally, it is used when a metal is present. Attach a prefix to the 2nd atom in the formula (always).Attach a prefix to the 1st atom in the formula (only if there is more than one of them).

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Name the following compounds using both the Prefix system and the Stock system:

FormulaN2O

NONO2

N2O3

N2O4

N2O5

IClCS2

SO2

PCl3

P2O5

SCl6

MnO2

Prefix System Namedinitrogen monoxidenitrogen monoxidenitrogen dioxidedinitrogen trioxidedinitrogen tetr(a)oxidedinitrogen pent(a)oxideiodine monochloridecarbon disulfidesulfur dioxidephosphorus trichloridediphosphorus pent(a)oxidesulfur hexachloridemanganese dioxide

Stock System Namenitrogen(I) oxidenitrogen(II) oxidenitrogen(IV) oxidenitrogen(III) oxidenitrogen(IV) oxidenitrogen(V) oxideiodine(I) chloridecarbon(IV) sulfidesulfur(IV) oxidephosphorus(III) chloridephosphorus(V) oxidesulfur(VI) chloridemanganese(IV) oxide

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The “Ous-Ic” SystemFor binary compounds in which the cation usually has only 2 oxidation states, the old “ous-ic” system is sometimes used. In a few cases, when the English name of the metal atom is awkward, the Latin name of the metal is used instead.Then the suffix “ous” is added for the lower oxidation number and “ic” for the higher oxidation number.

SymbolCuFePbSnAuHgPtCo

Latin Namecuprumferrumplumbumstannumaurum --- --- ---

Ion Charge & NameCu+ = cuprous, Cu+2 = cupricFe+2 = ferrous, Fe+3 = ferricPb+2 = plumbous, Pb+4 = plumbicSn+2 = stannous, Sn+4 = stannicAu+ = aurous, Au+3 = auricHg+ = mercurous, Hg+2 = mercuricPt+2 = platinous, Pt+4 = platinicCo+2 = cobaltous, Co+3 = cobaltic

Namecopperironleadtingoldmercuryplatinumcobalt

29

Name the following compounds using the “ous-ic” system.

FormulaPbCl2

PbCl4

SnBr2

SnBr4

Cu2O

CuOFeOFe2O3

Au2S3

PtF2

PtS2

Hg4C

Hg3N2

Ous-Ic Nameplumbous chlorideplumbic chloridestannous bromidestannic bromidecuprous oxidecupric oxideferrous oxideferric oxideauric sulfideplatinous fluorideplatinic sulfidemercurous carbidemercuric nitride

Stock System Namelead(II) chloridelead(IV) chloridetin(II) bromidetin(IV) bromidecopper(I) oxidecopper(II) oxideiron(II) oxideiron(III) oxidegold(III) sulfideplatinum(II) fluorideplatinum(IV) sulfidemercury(I) carbidemercury(II) nitride

30

Peroxides:• A reactive type of compound, called ‘peroxides’, has important commercial and industrial

applications. The most familiar example is hydrogen peroxide, H2O2.

O

HH

O

OH

H

H2Ohydrogen oxide

H2O2

hydrogen peroxide‘per’ means one more O than the normal oxide.

• H2O2 is one of the strongest oxidizers known.

• 35 – 50% aqueous solutions are used industrially for pulp and paper bleaching.

• Up to 12% H2O2 is used as hair bleach and 3% H2O2 is sold as a household disinfectant.

• Peroxides are unusual, in that the ‘O’ in a peroxide has an Ox # = -1 and the formula of the peroxide anion is written O2

-2 (because the peroxide anion is a bonded pair of O’s).

• Recall that ‘O’ is in Group 6A, it will be stable when it gains 2 electrons and becomes oxide, O-2, so it is not surprising that peroxide, O2

-2, is so reactive (unstable).

31

Group 1A and 2A metal peroxides have some interesting applications.For example, sodium peroxide, Na2O2, converts carbon dioxide to oxygen and sodium carbonate.

Na2O2 + CO2 Na2CO3 + ½ O2

Both lithium peroxide and sodium peroxide have been used to regenerate oxygen from exhaled air in confined spaces, such as submarines and spacecraft.Peroxide Practice: Write the name or formula of the following compounds. Spelling counts.

FormulaH2O

H2O2

BaO2

K2O2

K2O

CaO2

Stock System Namehydrogen oxide (Prefix name: dihydrogen monoxide)hydrogen peroxidebarium peroxidepotassium peroxidepotassium oxidecalcium peroxide

Ox # & ChargesH+ O-2

H+ O2-2

Ba+2 O2-2

K+ O2-2

K+ O-2

Ca+2 O2-2

Note that peroxide formulas, such as H2O2, Na2O2, etc. are not reduced to the lowest whole number ratio.Do not write HO or NaO. All peroxides contain a pair of bonded O’s.Finished Part 1.

32

Congrats, you just completed inorganic chemical nomenclature part 1 on Binary Compounds

There is also a second video dealing with the nomenclature of Polyatomic Compounds.

Youtube ‘Inorganic Chemical Nomenclature Part 2 Polyatomic Compounds’

33

Intro to Inorganic Chemical NomenclaturePart 2, Polyatomic Compounds

This lesson was divided into two partsPart 2 Polyatomic Compounds

• In this video we will study the nomenclature of Polyatomic Compounds

• There is also a first video in which I presented the nomenclature of Binary Compounds. You should complete that video first.

• Youtube ‘Inorganic Chemical Nomenclature Part 1 Binary Compounds’

34

Inorganic Nomenclature Part 2 Polyatomic CompoundsOxy Acids:Oxyacids contain H, O and another nonmetal atom. Many oxyacids are commonly found in cleaning products, fruits, food ingredients, industrial chemicals, etc.

• Phosphoric acid, H3PO4, is used to pickle steel and is the flavour in root beers and colas.

• Sulfuric acid, H2SO4, is the electrolyte in the automobile lead-acid battery (35% H2SO4).

• Carbonic acid, H2CO3, is formed when carbon dioxide, CO2, is dissolved in water (H2O + CO2 H2CO3). Carbonated beverages contain carbonic acid.

• A 5% solution of acetic acid, CH3COOH, in water is sold as vinegar.

35

Here are eight important oxyacids. Some of these exist with varying numbers of oxygen atoms. The ‘main’ oxyacids, the –ic acids, and their names are highlighted.

A Car Never Stays Perfectly Clean

When oxyacids react, they release hydrogen ions, H+, and leave behind polyatomic anions.HNO3 H+ + NO3

- and H2SO4 2H+ + SO4-2 and H3PO4 3H+ + PO4

-3

ic acidsper … ic

… ic… ous

hypo … ous

Acetic

CH3COOH

Carbonic

H2CO3

Nitric

HNO3

HNO2

Sulfuric

H2SO4

H2SO3

Phosphoric

H3PO4

H3PO3

H3PO2

ChloricHClO4

HClO3

HClO2

HClO

BromicHBrO4

HBrO3

HBrO2

HBrO

IodicHIO4

HIO3

HIO2

HIO

A Car Never Stays Perfectly Clean

ate anionsper … ate

… ate… ite

hypo … ite

Acetate

CH3COO-

Carbonate

CO3

-2

Nitrate

NO3

-

NO2-

Sulfate

SO4-2

SO3-2

Phosphate

PO4-3

* HPO3-2

** H2PO2-

ChlorateClO4

-

ClO3-

ClO2-

ClO-

BromateBrO4

-

BrO3-

BrO2-

BrO-

IodateIO4

-

IO3-

IO2-

IO-

* H3PO3 only has 2 acidic H’s, so phosphite is HPO3-2 ** H3PO2 only has 1 acidic H, so hypophosphite is H2PO2

-

36

-1+1 +

Practice: Study the structures and learn the formulas and names of the acids and their anions.

CH3COOHacetic acid

CH3COO-

acetate

+1 +2-2

H2CO3

carbonic acidCO3

-2

carbonate

+1 + -1

HNO3

nitric acidNO3

-

nitrate

+1 +2

-2

H2SO4

sulfuric acidSO4

-2

sulfate

+1 +3

-3

H3PO4

phosphoric acidPO4

-3

phosphate

+1 + -1

HClO3

chloric acid

ClO3-

chlorate

37

Practice: Study the Lewis structures and learn the formulas & names of the acids and their anions.

C

O

OH O H H+2 + C

O- O O -

CH3COOHacetic acid

CH3COO-

acetate

CH

H

H

C

O

O H CH

H

H

C

O

O -H+ +

H2CO3

carbonic acidCO3

-2

carbonate

N+ OO-

OH H+ + N+ O -

O-

O

HNO3

nitric acidNO3

-

nitrate

H2SO4

sulfuric acidSO4

-2

sulfate

S

O

O

OO HH H+ + S

O

O

O -- O2

H3PO4

phosphoric acidPO4

-3

phosphate

HClO3

chloric acid

ClO3-

chlorate

3P

O

OO

O

H

H

H H+ + P

O

O -- O

O -

Cl

O

OO H H+ + Cl

O

O -O

38

Other Polyatomic Ions: A few other important polyatomic ions are shown below.

HCNhydrocyanic acid

CN-

cyanide

H2Owater

OH-

hydroxide

NH3

ammoniaNH4

+

ammonium

+1 + 

-1

+1 + 

-1

+1+ 

+1

HCN, hydrogen cyanide is acidic. In water it is called hydrocyanic acid. Although it is a weak acid and has a sweet almond odour, it is highly toxic when ingested.HCN H+ + CN-

The formula of water, H2O, looks like other binary acids, but water is completely neutral. When a H+ ion is removed from water, hydroxide ion, OH-, a strong base is formed.

Ammonia, NH3, is a moderately strong base with a pungent odour – the smell of Windex. When NH3 reacts with H+, an ammonium cation, NH4

+, is formed: NH3 + H+ NH4+

NH4+ (ammonium ion) is the only polyatomic ion

listed that is a cation. Its ‘ium’ ending indicates that it is a cation. The polyatomic anions have endings ‘ate’, ‘ite’, and ‘ide’.

39

Other Polyatomic Ions: A few other important polyatomic ions are shown below.

HCNhydrocyanic acid

CN-

cyanide

H2Owater

OH-

hydroxide

NH3

ammoniaNH4

+

ammonium

HCN, hydrogen cyanide is acidic. In water it is called hydrocyanic acid. Although it is a weak acid and has a sweet almond odour, it is highly toxic when ingested.HCN H+ + CN-

The formula of water, H2O, looks like other binary acids, but water is completely neutral. When a H+ ion is removed from water, hydroxide ion, OH-, a strong base is formed.

Ammonia, NH3, is a moderately strong base with a pungent odour – the smell of Windex. When NH3 reacts with H+, an ammonium cation, NH4

+, is formed: NH3 + H+ NH4+

NH4+ (ammonium ion) is the only polyatomic ion

listed that is a cation. Its ‘ium’ ending indicates that it is a cation. The polyatomic anions have endings ‘ate’, ‘ite’, and ‘ide’.

H+ +C NH -C N

H+ +O HH -O H

NH H

H

+ H+

N+

H

H HH

40

Monoprotic and Polyprotic Acids:Acids like CH3COOH, HNO3, HNO2, HClO4, HClO3, HClO2, HClO, etc. have only one ionizable H+ ion per molecule; these are called monoprotic acids.The three H’s bonded to C in CH3COOH are not ionizable.

Acids like H2CO3, H2SO4, H2SO3 and H3PO4 can release more than one H+ ion per molecule; they are called polyprotic acids because they can release more than one H+ (proton).When polyprotic acids lose some but not all of their ionizable H’s, important polyatomic anions form.

H2CO3 H+ + HCO3

- H+ +H2SO4 H+ + HSO4

- H+ + H2SO3 H+ + HSO3

- H+ + H3PO4 H+ + H2PO4

- H+ + HPO4

-2 H+ +

HCO3-

CO3-2

HSO4-

SO4-2

HSO3-

SO3-2

H2PO4-

HPO4-2

PO4-3

bicarbonate or monohydrogen carbonatecarbonatebisulfate or monohydrogen sulfatesulfatebisulfite or monohydrogen sulfitesulfitedihydrogen phosphatemonohydrogen phosphatephosphate

41

The stepwise ionization of some polyprotic acids is shown.

H3PO4

phosphoric acidH2PO4

-

dihydrogen phosphate

H2PO4-

dihydrogen phosphateHPO4

-2

monohydrogen phosphate

HPO4-2

monohydrogen phosphatePO4

-3

phosphate

H2SO4

sulfuric acidHSO4

-

bisulfate

HSO4-

bisulfateSO4

-2

sulfate

H2SO3

sulfurous acid

HSO3-

bisulfite

P

O

OO

O

H

H

H H+ + P

O

O -O

O H

H

H+ + P

O

O -O

O -

HP

O

O -O

O H

H

P

O

O -O

O -

H H+ + P

O

O -- O

O -

S

O

O

OO HH H+ + S

O

O

O -OH

S

O

O

O -OH H+ + S

O

O

O -- O

S

O

OO HH H+ + S

O

O -OH

42

Formulas and Names Involving Polyatomic Ions:Compounds containing polyatomic ions are named the same as binary compounds. Formulas containing polyatomic ions are written the same as binary compounds, with one difference …

sodium chloride is NaClcalcium chloride is CaCl2

sodium hydroxide is NaOHcalcium hydroxide is Ca(OH)2

Parentheses are not placed around monatomic ions like Cl-, even when several are present in the formula.

Parentheses are placed around polyatomic ions like OH-, only when several are present in the formula.

Ammonium hydroxide, NH4OH, contains two polyatomic ions, the ammonium cation, NH4+, and

the hydroxide anion, OH-

In ammonium cyanide, NH4CN, the N atom occurs twice. They remain separate so that the both the ammonium cation, NH4

+, and the cyanide anion, CN-, are recognized.

43

Formula

Practice: Write names or formulas in the empty cells. Use the Stock System.

Zn(C2H3O2)2

Fe(C2H3O2)3

Cr(NO2)6

Mn(NO3)7

Al2(SO4)3

Al(HSO4)3

K2SO3

Fe(HSO3)2

Ni(ClO4)2

Sn(ClO3)2

Pb(ClO2)4

HgBrOCo(BrO3)3

Cr(BrO4)3

Namezinc acetateiron(III) acetatechromium(VI) nitritemanganese(VII) nitratealuminum sulfatealuminum bisulfatepotassium sulfiteiron(II) bisulfitenickel(II) perchloratetin(II) chloratelead(IV) chloritemercury(I) hypobromitecobalt(III) bromatechromium(III) perbromate

ions & Ox #’sZn+2 CH3COO-

Fe+3 CH3COO-

Cr+6 NO2-

Mn+7 NO3-

Al+3 SO4-2

Al+3 HSO4-

K+ SO3-2

Fe+2 HSO3-

Ni+2 ClO4-

Sn+2 ClO3-

Pb+4 ClO2-

Hg+ BrO-

Co+3 BrO3-

Cr+3 BrO4-

44

Practice: Write names or formulas in the empty cells. Use the Stock System.

FormulaSr(IO2)2

(NH4)2SO4

LiIOBe(IO3)2

Cu(BrO2)2

Al2(CO3)3

Cu(HCO3)2

Ba3(PO4)2

Cd(IO4)2

W(CN)6

Mo(CO3)3

V2(SO3)5

Pt3(PO4)4

Hg(HSO4)2

Namestrontium ioditeammonium sulfatelithium hypoioditeberyllium iodatecopper(II) bromitealuminum carbonatecopper(II) bicarbonatebarium phosphate cadmium periodatetungsten(VI) cyanidemolybdenum(VI) carbonatevanadium(V) sulfiteplatinum(IV) phosphatemercury(II) bisulfate

ions & Ox #’sSr+2 IO2

-

NH4+ SO4

-2

Li+ IO-

Be+2 IO3-

Cu+2 BrO2-

Al+3 CO3-2

Cu+2 HCO3-

Ba+2 PO4-3

Cd+2 IO4-

W+6 CN-

Mo+6 CO3-2

V+5 SO3-2

Pt+4 PO4-3

Hg+2 HSO4-

45

In most oxyacids, adding or subtracting O’s to a formula does not change the number of ionizable H’s.HNO3 and HNO2 are both monoprotic acids.

H2SO4 and H2SO3 are both diprotic acids.

HClO4, HClO3, HClO2 and HClO are all monoprotic acids.

The oxyacids of P are unique. H3PO4 is triprotic, but H3PO3 is only diprotic, and H3PO2 is monoprotic.

Examine the structures of these oxyacids and note that acidic H’s are bonded to O, not to P.

P

O

OO

O

H

H

H P

O

OO HH

H

P

O

O H

H

H

acidic Hbonded to O nonacidic H

not bonded to O

acidic H

H 3PO 4

phosphoric acidtriprotic

H 3PO 3

phosphorous aciddiprotic

H 3PO 2

hypophosphorous acidm onoprotic

46

Because phosphorous acid (H3PO3) has only two ionizable H’s, HPO3-2 is fully ionized and can be named

monohydrogen phosphite or simply ‘phosphite’.

H+

P

O

OO HH

H

-P

O

O -OH

H

H+- P

O

O -- O

H

H3PO3, phosphorous acid H2PO3-, dihydrogen phosphite HPO3

-2, monohydrogen phosphite or simply ‘phosphite’

Because hypophosphorous acid (H3PO2) has only one ionizable H, H2PO2- is fully ionized and can be named

dihydrogen hypophosphite or simply ‘hypophosphite’.

P

O

O H

H

H H+ + P

O

O -

H

H

H3PO2, hypophosphorous acid H2PO2-, dihydrogen hypophosphite

or simply ‘hypophosphite’

H3PO4, phosphoric acid H2PO4-, dihydrogen phosphate HPO4

-2, monohydrogen phosphate PO4-3, phosphate

P

O

OO

O

H

H

H H+- P

O

O -O

O H

H H+- P

O

O -O

O -

H H+- P

O

O -- O

O -

47

As we are seeing, there are several conventions for naming the anions of partly ionized polyprotic acids. The student has latitude here, however, any correct name must identify the compound unambiguously. Try naming the following compounds using more than one correct name.FormulaH3PO4

NaH2PO4

K2HPO4

LiH2PO3

Ag2HPO3

NaH2PO2

(NH4)2HPO4

(NH4)2HPO3

NH4H2PO4

(NH4)2KPO4

Namephosphoric acid or hydrogen phosphatesodium dihydrogen phosphate or monosodium phosphatepotassium monohydrogen phosphate or dipotassium phosphatelithium dihydrogen phosphite or monolithium phosphitesilver monohydrogen phosphite or silver phosphitesodium dihydrogen hypophosphite or sodium hyposphosphitediammonium monohydrogen phosphate or diammonium phosphatediammonium monohydrogen phosphite or ammonium phosphiteammonium dihydrogen phosphate or monoammonium phosphatediammonium potassium phosphate

ions & Ox #’sH+ PO4

-3

Na+ H2PO4-

K+ HPO4-2

Li+ H2PO3-

Ag+ HPO3-2

Na+ H2PO2-

NH4+ HPO4

-2

NH4+ HPO3

-2

NH4+ H2PO4

-

NH4+ K+ PO4

-3

The number of H’s need not be stated, provided the number of other cations is explicitly stated in the name.Prefixes like ‘di’ or ‘tri’ should only be used when partially ionized polyprotic acids are being named.

48

For compounds of monovalent cations (Li+, Na+, K+, NH4+, etc.) we have seen that there are several

acceptable names … e.g., K2HPO4 = dipotassium monohydrogen phosphate or potassium monohydrogen phosphate or dipotassium phosphateHowever, when polyvalent cations, like Ca+2, Al+3, etc. are combined with partially ionized acids, the convention is to state the number of H’s but not the number of polyvalent metal cations, as follows …

Ca(H2PO4)2

CaHPO4

Al(H2PO4)3

Al2(HPO4)3

Fe2(HPO4)3

SnHPO4

Pb(H2PO3)4

Pd(H2PO2)4

Pd(H2PO2)2

calcium dihydrogen phosphatecalcium monohydrogen phosphatealuminum dihydrogen phosphatealuminum monohydrogen phosphateiron(III) monohydrogen phosphatetin(II) monohydrogen phosphatelead(IV) dihydrogen phosphitepalladium(IV) dihydrogen hypophosphite or palladium(IV) hypophosphitepalladium(II) dihydrogen hypophosphite or palladium(II) hypophosphite

Ca+2 H2PO4-

Ca+2 HPO4-2

Al+3 H2PO4-

Al+3 HPO4-2

Fe+3 HPO4-2

Sn+2 HPO4-2

Pb+4 H2PO3-

Pd+4 H2PO2-

Pd+2 H2PO2-

49

Practice: Write the name or formula of the following compounds. Spelling counts.The column on the right will not be marked.

FormulaMg(CH3COO)2

(NH4)2SO4

Fe2(CO3)3

Ba(NO3)2

Mn(ClO2)7

Cd(IO4)2

AlH3

Be3N2

Hg(BrO)2

H 2SO3

HClO3

(NH4)2HPO4

Zn(H2PO2)2

Stock System Namemagnesium acetateammonium sulfateiron(III) carbonatebarium nitratemanganese(VII) chloritecadmium periodatealuminum hydrideberyllium nitridemercury(II) hypobromitesulfurous acidchloric acidammonium monohydrogen phosphate or diammonium phosphatezinc dihydrogen hypophosphite or zinc hypophosphite

Ox # & ChargesMg+2 CH3COO-

NH4+ SO4

-2

Fe+3 CO3-2

Ba+2 NO3-

Mn+7 ClO2-

Cd+2 IO4-

Al+3 H-

Be+2 N-3

Hg+2 BrO-

H+ SO3-2

H+ ClO3-

NH4+ HPO4

-2

Zn+2 H2PO2-

50

Other Common Acids: A few other inorganic acids are commonly encountered in the laboratory. Study the structures and names of these acids and their anions.

Mn

O

O

O

O H H+ + Mn

O

O

O

O -

Cr

O

O

O

O HH H+ +2 Cr

O

- O

O

O -

Cr

O

O

O

O CrH

O

O

O H H+ +2 Cr

O

- O

O

O Cr

O

O

O -

Permanganic acid, HMnO4, is monoprotic. Its potassium salt, potassium permanganate (KMnO4) is a dark purple-colored reagent that is often used in the lab as a strong oxidizing titrant. Mn is in its highest oxidation state, +7, (which contributes to its strength as an oxidizer).

Chromic acid, H2CrO4, is a diprotic acid and strong oxidizer. Its potassium salt, potassium chromate, K2CrO4, is used as an indicator for measurement of chloride by silver nitrate titration. Cr is in its highest oxidation state, +6, (which contributes to its strength as an oxidizer).

Dichromic acid, H2Cr2O7 is another strongly oxidizing diprotic acid. Its potassium salt, potassium dichromate ( K2Cr2O7) is a common lab reagent.Can you calculate the Ox # of Cr in it?

permanganic acid, HMnO4 permanganate, MnO4-

chromic acid, H2CrO4 chromate, CrO4-2

dichromic acid, H2Cr2O7 dichromate, Cr2O7-2

51

Potassium permanganate, KMnO4, is a very dark purple, crystalline solid. The permanganate ion, MnO4

-, is released when dissolved in water, giving rise to bright purple solutions.

Potassium chromate, K2CrO4, is a bright yellow, crystalline solid.Aqueous solutions of this reagent are bright yellow owing to the presence of the chromate ion, CrO4

-2.

Bright orange potassium dichromate, K2Cr2O7, when dissolved in water, releases the dichromate ion, Cr2O7

-2.

52

Practice: Write the name or formula of the following compounds. Spelling counts.

FormulaFe(MnO4)3

Ag2CrO4

ZnCr2O7

Al2(CrO4)3

Na2Cr2O7

V2(Cr2O7)5

Mn2(SO4)7

Cr(PO4)2

Mo(MnO4)6

Cd(IO4)2

Co(BrO3)3

Ni(ClO2)2

Mg(BrO)2

Stock System Nameiron(III) permanganatesilver chromatezinc dichromatealuminum chromatesodium dichromatevanadium(V) dichromatemanganese(VII) sulfatechromium(VI) phosphatemolybdenum(VI) permanganatecadmium periodatecobalt(III) bromatenickel(II) chloritemagnesium hypobromite

Ox # & ChargesFe+3 MnO4

-

Ag+ CrO4-2

Zn+2 Cr2O7-2

Al+3 CrO4-2

Na+ Cr2O7-2

V+5 Cr2O7-2

Mn+7 SO4-2

Cr+6 PO4-3

Mo+6 MnO4-

Cd+2 IO4-

Co+3 BrO3-

Ni+2 ClO2-

Mg+2 BrO- Almost Finished

53

Name the following compounds using the “ous-ic” system.

FormulaPbCl2

PbCl4

SnBr2

SnBr4

Cu2O

CuOFeOFe2O3

Au2S3

PtF2

Pt(NO3)4

Hg(ClO4)2

Hg2SO3

Ous-Ic Nameplumbous chlorideplumbic chloridestannous bromidestannic bromidecuprous oxidecupric oxideferrous oxideferric oxideauric sulfideplatinous fluorideplatinic nitratemercuric perchloratemercurous sulfite

Stock System Namelead(II) chloridelead(IV) chloridetin(II) bromidetin(IV) bromidecopper(I) oxidecopper(II) oxideiron(II) oxideiron(III) oxidegold(III) sulfideplatinum(II) fluorideplatinum(IV) nitratemercury(II) perchloratemercury(I) sulfite

54

Congrats, you just completed inorganic chemical nomenclature part 2 on Polyatomic Compounds

There is also a previous video dealing with the nomenclature of Binary Compounds.

Youtube ‘Inorganic Chemical Nomenclature Part 1 Binary Compounds’